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For $\large A\, + \,B\, \rightleftharpoons \,C + D$ , $\large \Delta H\, = \, - QKJ$ , K_f and K_b respectively are 0.25 and 5000 at 400K. Now, K_c for same process at 500K may be

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$5.2 \times 10^{- 5}$

$4.5 \times 10^{- 4}$

$5 \times 10^{- 5}$

$4 \times 10^{- 5}$

answer is A.

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Detailed Solution

A + B $⇌$ C + D, ΔH = -QKJ

At 400 K K_f = 0.25; K_b = 5000

\large {K_{eq}} = \frac{{0.25}}{{5000}} = 5 \times {10^{ - 5}}

The reaction is exothermic at higher temperature, 500 K value of K_eq will be lesser than $\large 5 \times {10^{ - 5}}$

By inspection option (1) is the only value which is lesser than $\large 5 \times {10^{ - 5}}$

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